A galvanic cell is powered by the following redox reaction: 2Fe + 3(aq) + H2 (g) + 2OH−(aq) → 2Fe + 2(aq) + 2H2O(l)Answer the following questions about this cell. (a) Write a balanced equation for the half-reaction that takes place at the cathode. (b) Write a balanced equation for the half-reaction that takes place at the anode. (c) Calculate the cell voltage under standard conditions.

0.77V

Explanation:

The balanced anode and cathode half reaction equations are shown in the image attached. Reduction occurs at the cathode while oxidation occurs at the anode. Recall that hydrogen is a reference electrode hence its reduction potential is arbitrarily chosen as 0.00V under standard conditions. The hydroxide ion shows that the metal ion was maintained under alkaline conditions.

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2